Rate of Reaction Problem: Calculating Concentrations Before Reactions Occur

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SUMMARY

The discussion focuses on calculating the concentrations of KI, (NH4)2S2O8, and Na2S2O3 after mixing specific volumes and molarities of these solutions before any reaction occurs. The key conclusion is that the concentration of KI after mixing should equal 0.016 M. Participants emphasize treating the problem as a dilution calculation, where the moles of each reactant are determined and the final volume of the mixture is used to find the resulting concentrations.

PREREQUISITES
  • Understanding of molarity and dilution calculations
  • Basic knowledge of chemical reactions and stoichiometry
  • Familiarity with the concept of moles in chemistry
  • Ability to perform unit conversions and volume calculations
NEXT STEPS
  • Study dilution calculations in detail
  • Learn about stoichiometry in chemical reactions
  • Explore the concept of moles and their significance in reactions
  • Review the principles of reaction kinetics and rate laws
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Chemistry students, educators, and anyone involved in laboratory work or chemical analysis who needs to understand concentration calculations before reactions occur.

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Homework Statement


Assume that you mixed 20.00 mL of 0.040 M KI with 20.00 mL of 0.060 M (NH4)2SO8, 10.00 mL of 0.00070M Na2S2O3, and a few drops of starch. The point of mixing sets time=0. Calculate the concentrations of the three species KI, (NH4)2S2O8, and Na2S2O3 after mixing but before any reaction has occurred. Hint: your calculated [KI] should equal 0.016M.

Homework Equations


[tex]k= Ae^{-Ea/RT}[/tex]


The Attempt at a Solution


I don't really know how to start this problem. How can I calculate concentrations before reactions take place? Any help/hints will be much appreciated.
 
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Hello!
Work out the moles of each that have been added, and work out the overall volume of the mixture. The fraction will give you the concentration.
Ignoring the 'drops' of starch, which you have to do anyway, as there is no volume specified. That equation supplied isn't relevant, as far as I am aware.
I hope that helps!
 
As nobahar wrote - treat it as a simple dilution problem. You know initial concentrations and initial volumes, you can calculate final volume - that's all you need.

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